1. Chapter 3: Atoms-The Building Blocks of Matter
Section 1: The Atom – From Philosophical Idea to Scientific Theory

2. Lesson Starter Young people should not smoke.
Smoking at an early age may make it more difficult to quit smoking later.
Which of the above statements is an opinion and which is a theory?
Lesson Starter

3. Explain the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.
Summarize the five essential points of Dalton’s atomic theory.
Explain the relationship between Dalton’s atomic theory and the law of conservation of mass, the law of definite proportions, and the law of multiple proportions.
Objectives

4. DEMOCRITUS called nature’s basic particle an ATOM based on the Greek word meaning “INDIVISIBLE.”
ARISTOTLE did not believe in atoms. He believed that matter was continuous and this was accepted for nearly 2000 years.
Neither view was based on or supported by EXPERIMENTAL EVIDENCE.
Philosophical Ideas

5. Foundations of Atomic Theory
The TRANSFORMATION of a substance or substances into one or more NEW SUBSTANCES is known as a CHEMICAL REACTION.
Law of CONSERVATION OF MASS: MASS is neither CREATED NOR DESTROYED during ordinary chemical reactions or physical changes.
Foundations of Atomic Theory

6. Foundations of Atomic Theory
Law of DEFINITE PROPORTIONS: a chemical COMPOUND contains the SAME ELEMENTS in exactly the SAME PROPORTION by MASS regardless of the size of the sample or the source of the compound.
it doesn’t matter how or where a pure chemical compound is prepared, it is made of a fixed proportion of elements
sodium chloride is ALWAYS made of 39.34% SODIUM and % CHLORINE, by mass
Foundations of Atomic Theory

7. Foundations of Atomic Theory
Law of MULTIPLE PROPORTIONS: if two or more DIFFERENT COMPOUNDS are composed of the SAME TWO ELEMENTS then the RATIO of the masses of the SECOND ELEMENT combined with a certain mass of the FIRST ELEMENT is always a ratio of SMALL WHOLE NUMBERS
carbon forms two compounds with oxygen, CO and CO2
In carbon dioxide, for every 1.00 g of carbon, it is combined with 2.66 g of oxygen.
In carbon monoxide, for every 1.00 g of carbon, it is combined with 1.33 g of oxygen.
the ratio of the oxygen in the compounds is 2.66 to 1.33 or 2:1.
Foundations of Atomic Theory

8. Dalton’s Atomic Theory
All matter is composed of EXTREMELY SMALL PARTICLES called ATOMS.
Atoms of a given element are IDENTICAL in SIZE, MASS, and other PROPERTIES; atoms of different elements DIFFER in size, mass, and other properties.
Dalton’s Atomic Theory

9. Dalton’s Atomic Theory
Atoms cannot be SUBDIVIDED, CREATED, OR DESTROYED.
Atoms of different elements combine in SIMPLE WHOLE NUMBER RATIOS to form chemical COMPOUNDS.
In chemical reactions, atoms are COMBINED, SEPARATED, OR REARRANGED.
Dalton’s Atomic Theory

10. LAW OF CONSERVATION OF MASS: Chemical reactions involve the combination, separation, or rearrangement of atoms. Atoms are not subdivided, created, or destroyed.
LAW OF DEFINITE PROPORTIONS: A given chemical compound is always composed of the same combination of atoms.
LAW OF MULTIPLE PROPORTIONS: carbon dioxide always contains twice as many atoms of oxygen as does carbon monoxide.
The Laws Explained

11. Not all aspects of Dalton’s atomic theory have proven to be correct
Not all aspects of Dalton’s atomic theory have proven to be correct. We now know that:
Atoms are DIVISIBLE into even smaller particles.
A given element can have atoms with different MASSES.
Modern Atomic Theory

12. Modern Atomic Theory Some important concepts remain unchanged.
All MATTER is composed of ATOMS.
ATOMS of any one element DIFFER in PROPERTIES from atoms of another element.
Modern Atomic Theory